AP* CHEMISTRY EQUATIONS BY TYPE
|
|
- Hillary Ellis
- 7 years ago
- Views:
Transcription
1 Created by Kristen Henry Jones 2/25/2009 AP* CHEMISTRY EQUATIONS BY TYPE Double Replacement 1. Hydrogen sulfide is bubbled through a solution of silver nitrate. 2. An excess of sodium hydroxide solution is added to a solution of magnesium nitrate. 3. Solutions of sodium iodide and lead nitrate are mixed. 4. A solution of ammonia is added to a solution of ferric chloride. 5. Solutions of silver nitrate and sodium chromate are mixed. 6. Excess silver acetate is added to a solution of trisodium phosphate. 7. Manganese(II) nitrate solution is mixed with sodium hydroxide solution. 8. A saturated solution of calcium hydroxide is added to a solution of magnesium chloride. 9. Hydrogen sulfide gas is added to a solution of cadmium nitrate. 10. Dilute sulfuric acid is added to a solution of barium acetate. 11. A precipitate is formed when solutions of trisodium phosphate and calcium chloride are mixed. 12. A solution of copper(ii) sulfate is added to a solution of barium hydroxide. 13. Equal volumes of dilute equimolar solutions of sodium carbonate and hydrochloric acid are mixed. 14. Solid barium peroxide is added to cold dilute sulfuric acid. 15. Excess hydrochloric acid solution is added to a solution of potassium sulfite. 16. Dilute sulfuric acid is added to a solution of barium chloride. 17. A solution of sodium hydroxide is added to a solution of ammonium chloride. 18. Dilute hydrochloric acid is added to a solution of potassium carbonate. 19. Gaseous hydrogen sulfide is bubbled through a solution of nickel(ii) nitrate. 20. A solution of sodium sulfide is added to a solution of zinc nitrate. 21. Concentrated hydrochloric acid is added to solid manganese(ii) sulfide. 22. Solutions of tripotassium phosphate and zinc nitrate are mixed. 23. Dilute acetic acid solution is added to solid magnesium carbonate. 24. Gaseous hydrofluoric acid reacts with solid silicon dioxide. 25. Equimolar amounts of trisodium phosphate and hydrogen chloride, both in solution, are mixed. 26. Ammonium chloride crystals are added to a solution of sodium hydroxide. 27. Hydrogen sulfide gas is bubbled through a solution of lead(ii) nitrate. 28. Solutions of silver nitrate and sodium chromate are mixed. 29. Solutions of sodium fluoride and dilute hydrochloric acid are mixed. 30. A saturated solution of barium hydroxide is mixed with a solution of iron(iii) sulfate. 31. A solution of ammonium sulfate is added to a potassium hydroxide solution. 32. A solution of ammonium sulfate is added to a saturated solution of barium hydroxide. 33. Dilute sulfuric acid is added to solid calcium fluoride. 34. Dilute hydrochloric acid is added to a dilute solution of mercury(i) nitrate. 35. Dilute sulfuric acid is added to a solution of lithium hydrogen carbonate. 36. Dilute hydrochloric acid is added to a solution of potassium sulfite. 37. Carbon dioxide gas is bubbled through water containing a suspension of calcium carbonate. 38. Excess concentrated sulfuric acid is added to solid calcium phosphate. 39. Hydrogen sulfide gas is bubbled into a solution of mercury(ii) chloride. AP and Advanced Placement Program are registered trademarks of the College Entrance Examination Board, which was not involved in the production of and does not endorse this product. 1
2 40. Solutions of zinc sulfate and sodium phosphate are mixed. 41. Solutions of silver nitrate and lithium bromide are mixed. 42. Solutions of manganese(ii) sulfate and ammonium sulfide are mixed. 43. Excess hydrochloric acid solution is added to a solution of potassium sulfite. Single Replacement 1. A piece of aluminum metal is added to a solution of silver nitrate. 2. Aluminum metal is added to a solution of copper(ii) chloride. 3. Hydrogen gas is passed over hot copper(ii) oxide. 4. Small chunks of solid sodium are added to water. 5. Calcium metal is added to a dilute solution of hydrochloric acid. 6. Magnesium turnings are added to a solution of iron(iii) chloride. 7. Chlorine gas is bubbled into a solution of sodium bromide. 8. A strip of magnesium is added to a solution of silver nitrate. 9. Solid calcium is added to warm water. 10. Liquid bromine is added to a solution of potassium iodide. 11. Chlorine gas is bubbled into a solution of potassium iodide. 12. Lead foil is immersed in silver nitrate solution. 13. Solid zinc strips are added to a solution of copper(ii) sulfate. 14. Sodium metal is added to water. 15. A bar of zinc metal is immersed in a solution of copper(ii) sulfate. 16. A small piece of sodium metal is added to distilled water. Anhydrides 1. Excess water is added to solid calcium hydride. 2. Solid lithium hydride is added to water. 3. Liquid phosphorus trichloride is poured into a large excess of water. 4. Solid sodium carbide is added to an excess of water. 5. Solid magnesium nitride is added to excess deuterium oxide. 6. Water is added to a sample of pure phosphorus tribromide. 7. Water is added to a sample of pure sodium hydride. 8. Dinitrogen trioxide gas is bubbled into water. 9. Solid phosphorus pentachloride is added to excess water. 10. Solid dinitrogen pentoxide is added to water. 11. Sulfur trioxide gas is added to excess water. 12. Solid sodium oxide is added to water. 13. Phosphorus(V) oxytrichloride is added to water. 14. Water is added to a sample of solid magnesium nitride. 15. Solid potassium oxide is added to water. 16. Solid sodium cyanide is added to water. 17. Trisodium phosphate crystals are added to water. 18. Solid lithium oxide is added to excess water. 19. Solid barium oxide is added to distilled water. 20. Solid calcium hydride is added to distilled water. 21. Phosphorous(V) oxide powder is sprinkled over distilled water. Created by Kristen Henry Jones 2/25/ AP and Advanced Placement Program are registered trademarks of the College Entrance Examination Board, which was not involved in the production of and does not endorse this product.
3 Combustion 1. Lithium metal is burned in air. 2. The hydrocarbon hexane is burned in excess oxygen. 3. Gaseous diborane, B 2 H 6, is burned in excess oxygen. 4. A piece of solid bismuth is heated strongly in oxygen. 5. Solid zinc sulfide is heated in an excess of oxygen. 6. Propanol is burned completely in air. 7. Excess oxygen gas is mixed with ammonia gas in the presence of platinum. 8. Gaseous silane, SiH 4, is burned in oxygen. 9. Ethanol is completely burned in air. 10. Solid copper(ii) sulfide is heated strongly in oxygen gas. 11. Ethanol is burned in oxygen. 12. Carbon disulfide vapor is burned in excess oxygen. Redox 1. Iron(III) ions are reduced by iodide ions. 2. Potassium permanganate solution is added to concentrated hydrochloric acid. 3. Magnesium metal is added to dilute nitric acid, giving as one of the products a compound in which the oxidation number for nitrogen is A solution of potassium iodide is electrolyzed. 5. Potassium dichromate solution is added to an acidified solution of sodium sulfite. 6. Solutions of potassium iodide, potassium iodate, and dilute sulfuric acid are mixed. 7. A solution of tin(ii) sulfate is added to a solution of iron(iii) sulfate. 8. Metallic copper is heated with concentrated sulfuric acid. 9. Manganese(IV) oxide is added to warm, concentrated hydrobromic acid. 10. Chlorine gas is bubbled into cold dilute sodium hydroxide. 11. Solid iron(iii) oxide is heated in excess carbon monoxide. 12. Hydrogen peroxide solution is added to acidified potassium iodide solution. 13. Hydrogen peroxide is added to an acidified solution of potassium dichromate. 14. Sulfur dioxide gas is bubbled through an acidified solution of potassium permanganate. 15. A solution containing tin(ii) ions is added to an acidified solution of potassium dichromate. 16. Solid silver sulfide is warmed with dilute nitric acid. 17. A dilute solution of sulfuric acid is electrolyzed between platinum electrodes. 18. Pellets of lead are dropped into hot sulfuric acid. 19. Potassium permanganate solution is added to a solution of oxalic acid, H 2 C 2 O 4, acidified with a few drops of sulfuric acid. 20. Powdered iron is added to a solution of iron(iii) sulfate. 21. A concentrated solution of hydrochloric acid is added to powdered manganese dioxide and gently heated. 22. A strip of copper metal is added to a concentrated solution of sulfuric acid. 23. Copper(II) sulfide is oxidized by dilute nitric acid. 24. A solution of copper(ii) sulfate is electrolyzed using inert electrodes. 25. A solution of potassium iodide is added to an acidified solution of potassium dichromate. 26. Hydrogen peroxide solution is added to a solution of iron(ii) sulfate. 27. Solid silver is added to a dilute nitric acid(6m) solution. Created by Kristen Henry Jones 2/25/ AP and Advanced Placement Program are registered trademarks of the College Entrance Examination Board, which was not involved in the production of and does not endorse this product.
4 28. A solution of formic acid, HCOOH, is oxidized by an acidified solution of potassium dichromate. 29. A piece of iron is added to a solution of iron(iii) sulfate. 30. An acidified solution of potassium permanganate is added to a solution of sodium sulfite. 31. A solution of tin(ii) chloride is added to a solution of iron(iii) sulfate. 32. Concentrated hydrochloric acid solution is added to solid manganese(iv) oxide and the reactants are heated. 33. A strip of copper is immersed in dilute nitric acid. 34. Potassium permanganate solution is added to an acidic solution of hydrogen peroxide. 35. Solid copper is added to a dilute nitric acid solution. 36. Chlorine gas is bubbled into a cold solution of dilute sodium hydroxide. 37. A solution of potassium permanganate is mixed with an alkaline solution of sodium sulfite. 38. Solid sodium dichromate is added to an acidified solution of sodium iodide. 39. Hydrogen gas is passed over hot iron(iii) oxide. 40. Solutions of potassium iodide and potassium iodate are mixed in acid solution. 41. Hydrogen peroxide is added to an acidified solution of sodium bromide. 42. Chlorine gas is bubbled into a cold, dilute solution of potassium hydroxide. 44. A solution of iron(ii) nitrate is exposed to air for an extended period of time. 45. A stream of chlorine gas is passed through a solution of cold, dilute sodium hydroxide. 46. A solution of tin(ii) chloride is added to an acidified solution of potassium permanganate. 47. A concentrated solution of hydrochloric acid is added to solid potassium permanganate. 48. A solution of potassium dichromate is added to an acidified solution of iron(ii) chloride. AcidBase Neutralizations 1. Solutions of ammonia and hydrofluoric acid are mixed. 2. Hydrogen sulfide gas is bubbled through a solution of potassium hydroxide. 3. A solution of sulfuric acid is added to a solution of barium hydroxide until the same number of moles of each compound has been added. 4. A solution of sodium hydroxide is added to a solution of sodium dihydrogen phosphate until the same number of moles of each compound has been added. 5. Dilute nitric acid is added to crystals of pure calcium oxide. 6. Equal volumes of 0.1molar sulfuric acid and 0.1molar potassium hydroxide are mixed. 7. A solution of ammonia is added to a dilute solution of acetic acid. 8. Excess sulfur dioxide gas is bubbled through a dilute solution of potassium hydroxide. 9. Sulfur dioxide gas is bubbled into an excess of a saturated solution of calcium hydroxide. 10. A solution of sodium hydroxide is added to a solution of calcium hydrogen carbonate until the number of moles of sodium hydroxide added is twice the number of moles of the calcium salt. 11. Equal volumes of 0.1M hydrochloric acid and 0.1M sodium monohydrogen phosphate are mixed. 12. Hydrogen sulfide gas is bubbled through excess potassium hydroxide solution. 13. Ammonia gas and carbon dioxide gas are bubbled into water. 14. Carbon dioxide gas is bubbled through a concentrated solution of sodium hydroxide. 15. Acetic acid solution is added to a solution of sodium hydrogen carbonate. Created by Kristen Henry Jones 2/25/ AP and Advanced Placement Program are registered trademarks of the College Entrance Examination Board, which was not involved in the production of and does not endorse this product.
5 16. Excess potassium hydroxide solution is added to a solution of potassium dihydrogen phosphate. 17. Carbon dioxide gas is bubbled through a concentrated solution of potassium hydroxide. Complex Ions 1. Concentrated(15M) ammonia solution is added in excess to a solution of copper(ii) nitrate. 2. An excess of nitric acid solution is added to a solution of tetraaminecopper(ii) sulfate. 3. Dilute hydrochloric acid is added to a solution of diamminesilver(i) nitrate. 4. Solid aluminum nitrate is dissolved in water. 5. A suspension of copper(ii) hydroxide is treated with an excess of ammonia water. 6. A solution of diamminesilver(i) chloride is treated with dilute nitric acid. 7. An excess of concentrated ammonia solution is added to freshly precipitate copper(ii) hydroxide. 8. Excess dilute nitric acid is added to a solution containing the tetraaminecadmium(ii) ion. 9. An excess of ammonia is bubbled through a solution saturated with silver chloride. 10. Solid aluminum oxide is added to a solution of sodium hydroxide. 11. A concentrated solution of ammonia is added to a solution of zinc iodide. 12. An excess of sodium hydroxide solution is added to a solution of aluminum chloride. 13. A concentrated solution of ammonia is added to a solution of copper(ii) chloride. 14. Excess concentrated sodium hydroxide solution is added to solid aluminum hydroxide. 15. Excess concentrated ammonia solution is added to a suspension of silver chloride, 16. Pellets of aluminum metal are added to a solution containing an excess of sodium hydroxide. 17. A suspension of zinc hydroxide is treated with concentrated sodium hydroxide solution. 18. Silver chloride is dissolved in excess ammonia solution. 19. Sodium hydroxide solution is added to a precipitate of aluminum hydroxide in water. 20. A drop of potassium thiocyanate is added to a solution of iron(iii) chloride. 21. A concentrated solution of ammonia is added to a suspension of zinc hydroxide. 22. Excess concentrated potassium hydroxide solution is added to a precipitate of zinc hydroxide. 23. A solution of ammonium thiocyanate is added to a solution of iron(iii) chloride. 24. Excess sodium cyanide is added to a solution of silver nitrate. Addition 1. The gases boron trifluoride and ammonia are mixed. 2. A mixture of solid calcium oxide and solid tetraphosphorus decaoxide is heated. 3. Solid calcium oxide is exposed to a stream of carbon dioxide gas. 4. Solid calcium oxide is heated in the presence of sulfur trioxide gas. 5. Calcium metal is heated strongly in nitrogen gas. 6. Excess chlorine gas is passed over hot iron filings. 7. Powdered magnesium oxide is added to a container of carbon dioxide gas. 8. A piece of lithium metal is dropped into a container of nitrogen gas. 9. Magnesium metal is burned in nitrogen gas. 10. Sulfur dioxide gas is passed over solid calcium oxide. 11. Samples of boron trichloride gas and ammonia gas are mixed. Created by Kristen Henry Jones 2/25/ AP and Advanced Placement Program are registered trademarks of the College Entrance Examination Board, which was not involved in the production of and does not endorse this product.
6 Decomposition 1. A solution of hydrogen peroxide is heated. 2. Solid magnesium carbonate is heated. 3. A solution of hydrogen peroxide is catalytically decomposed. 4. Solid potassium chlorate is heated in the presence of manganese dioxide as a catalyst. 5. Sodium hydrogen carbonate is dissolved in water. 6. Solid ammonium carbonate is heated. Created by Kristen Henry Jones 2/25/ AP and Advanced Placement Program are registered trademarks of the College Entrance Examination Board, which was not involved in the production of and does not endorse this product.
7 KEY TO AP CHEMISTRY EQUATIONS BY TYPE , , , 1995 Double Replacement 1. Hydrogen sulfide is bubbled through a solution of silver nitrate. H 2 S + Ag 1+! Ag 2 S + H + 2. An excess of sodium hydroxide solution is added to a solution of magnesium nitrate. OH + Mg 2+! Mg(OH) 2 3. Solutions of sodium iodide and lead nitrate are mixed. I + Pb 2+! PbI 2 4. A solution of ammonia is added to a solution of ferric chloride. NH 3 + H 2 O + Fe 3+! NH Fe(OH) 3 5. Solutions of silver nitrate and sodium chromate are mixed. Ag + + CrO 4 2! Ag 2 CrO 4 6. Excess silver acetate is added to a solution of trisodium phosphate. Ag + + PO 4 3! Ag 3 PO 4 7. Manganese(II) nitrate solution is mixed with sodium hydroxide solution. Mn 2+ + OH! Mn(OH) 2 8. A saturated solution of calcium hydroxide is added to a solution of magnesium chloride. Mg 2+ + OH! Mg(OH) 2 9. Hydrogen sulfide gas is added to a solution of cadmium nitrate. H 2 S + Cd 2+! CdS + H Dilute sulfuric acid is added to a solution of barium acetate. H + + SO Ba 2+ + C 2 H 3 O 2! BaSO 4 + HC 2 H 3 O A precipitate is formed when solutions of trisodium phosphate and calcium chloride are mixed. PO Ca 2+!Ca 3 (PO 4 ) A solution of copper(ii) sulfate is added to a solution of barium hydroxide. Cu 2+ + SO Ba 2+ + OH! Cu(OH) 2 + BaSO Equal volumes of dilute equimolar solutions of sodium carbonate and hydrochloric acid are mixed. H + + CO 3 2! HCO Solid barium peroxide is added to cold dilute sulfuric acid. BaO 2 +H + + SO 4 2! BaSO 4 + H 2 O Excess hydrochloric acid solution is added to a solution of potassium sulfite. H + + SO 3 2! H 2 O + SO Dilute sulfuric acid is added to a solution of barium chloride. SO Ba 2+! BaSO A solution of sodium hydroxide is added to a solution of ammonium chloride. NH OH! NH 3 + H 2 O 18. Dilute hydrochloric acid is added to a solution of potassium carbonate. H + + CO 3 2! H 2 O + CO Gaseous hydrogen sulfide is bubbled through a solution of nickel(ii) nitrate. H 2 S + Ni 2+! NiS + H A solution of sodium sulfide is added to a solution of zinc nitrate. Kristen Henry Jones 1
8 S 2 + Zn 2+! ZnS 21. Concentrated hydrochloric acid is added to solid manganese(ii) sulfide. H + + MnS! H 2 S + Mn Solutions of tripotassium phosphate and zinc nitrate are mixed. PO Zn 2+! Zn 3 (PO 4 ) Dilute acetic acid solution is added to solid magnesium carbonate. HC 2 H 3 O 2 + MgCO 3! H 2 O + CO 2 + Mg 2+ + C 2 H 3 O Gaseous hydrofluoric acid reacts with solid silicon dioxide. HF + SiO 2! H 2 O + SiF Equimolar amounts of trisodium phosphate and hydrogen chloride, both in solution, are mixed. PO H +! HPO Ammonium chloride crystals are added to a solution of sodium hydroxide. NH 4 Cl + OH! NH 3 + H 2 O + Cl 27. Hydrogen sulfide gas is bubbled through a solution of lead(ii) nitrate. H 2 S + Pb 2+! PbS + H Solutions of silver nitrate and sodium chromate are mixed. Ag + + CrO 4 2! Ag 2 CrO Solutions of sodium fluoride and dilute hydrochloric acid are mixed. F + H +! HF 30. A saturated solution of barium hydroxide is mixed with a solution of iron(iii) sulfate. Ba 2+ + OH + Fe 3+ + SO 4 2! BaSO 4 + Fe(OH) A solution of ammonium sulfate is added to a potassium hydroxide solution. NH OH! NH 3 + H 2 O 32. A solution of ammonium sulfate is added to a saturated solution of barium hydroxide. NH SO Ba 2+ +OH! NH 3 + H 2 O + BaSO Dilute sulfuric acid is added to solid calcium fluoride. H + + SO CaF 2! CaSO 4 + HF 34. Dilute hydrochloric acid is added to a dilute solution of mercury(i) nitrate. Cl + Hg 2 2+! Hg 2 Cl Dilute sulfuric acid is added to a solution of lithium hydrogen carbonate. H + + HCO 3! H 2 O + CO Dilute hydrochloric acid is added to a solution of potassium sulfite. H + + SO 3 2! H 2 O + SO Carbon dioxide gas is bubbled through water containing a suspension of calcium carbonate. CO 2 + CaCO 3 + H 2 O! HCO 3 + Ca Excess concentrated sulfuric acid is added to solid calcium phosphate. H 2 SO 4 + Ca 3 (PO 4 ) 2! H 3 PO 4 + CaSO 4 (or Ca 2+ + SO 4 2 ) 39. Hydrogen sulfide gas is bubbled into a solution of mercury(ii) chloride. H 2 S + Hg 2+! HgS + H + SingleReplacement 1. A piece of aluminum metal is added to a solution of silver nitrate. Kristen Henry Jones 2
9 Al + Ag +! Al 3+ + Ag 2. Aluminum metal is added to a solution of copper(ii) chloride. Al + Cu 2+! Al 3+ + Cu 3. Hydrogen gas is passed over hot copper(ii) oxide. H 2 + CuO! H 2 O + Cu 4. Small chunks of solid sodium are added to water. Na + H 2 O! Na + + OH + H 2 5. Calcium metal is added to a dilute solution of hydrochloric acid. Ca + H +! Ca 2+ + H 2 6. Magnesium turnings are added to a solution of iron(iii) chloride. Mg + Fe 3+! Mg 2+ + Fe 7. Chlorine gas is bubbled into a solution of sodium bromide. Cl 2 + Br! Cl + Br 2 8. A strip of magnesium is added to a solution of silver nitrate. Mg + Ag +! Mg 2+ + Ag 9. Solid calcium is added to warm water. Ca + H 2 O! Ca 2+ + OH + H Liquid bromine is added to a solution of potassium iodide. Br 2 + I! Br + I Chlorine gas is bubbled into a solution of potassium iodide. Cl 2 + I! Cl + I Lead foil is immersed in silver nitrate solution. Pb + Ag +! Pb 2+ + Ag 13. Solid zinc strips are added to a solution of copper(ii) sulfate. Zn + Cu 2+! Zn 2+ + Cu 14. Sodium metal is added to water. Na + H 2 O! Na + + OH + H A bar of zinc metal is immersed in a solution of copper(ii) sulfate. Zn + Cu 2+! Zn 2+ + Cu Anhydrides 1. Excess water is added to solid calcium hydride. H 2 O + CaH 2! Ca 2+ + OH or (Ca(OH) 2 )+ H 2 2. Solid lithium hydride is added to water. LiH + H 2 O! Li + + OH + H 2 3. Liquid phosphorus trichloride is poured into a large excess of water. PCl 3 + H 2 O! H 3 PO 3 + H + + Cl 4. Solid sodium carbide is added to an excess of water. Na 4 C + H 2 O! C 2 H 2 + Na + + OH 5. Solid magnesium nitride is added to excess deuterium oxide. Mg 3 N 2 + D 2 O! Mg(OD) 2 + ND 3 6. Water is added to a sample of pure phosphorus tribromide. H 2 O + PBr 3! H 3 PO 3 + H + + Br 7. Water is added to a sample of pure sodium hydride. Kristen Henry Jones 3
10 H 2 O + NaH! Na + + OH + H 2 8. Dinitrogen trioxide gas is bubbled into water. N 2 O 3 + H 2 O! HNO 2 9. Solid phosphorus pentachloride is added to excess water. PCl 5 + H 2 O! H3 PO 4 + H+ + Cl 10. Solid dinitrogen pentoxide is added to water. N 2 O 5 + H 2 O! H + + NO Sulfur trioxide gas is added to excess water. SO 3 + H 2 O! H + + SO Solid sodium oxide is added to water. Na 2 O + H 2 O! Na + + OH 13. Phosphorus(V) oxytrichloride is added to water. POCl 3 + H 2 O! H 3 PO 4 + H + + Cl 14. Water is added to a sample of solid magnesium nitride. H 2 O + Mg 3 N 2!Mg(OH) 2 + NH Solid potassium oxide is added to water. K 2 O + H 2 O! K + + OH 16. Solid sodium cyanide is added to water. NaCN + H 2 O! HCN + Na + + OH 17. Trisodium phosphate crystals are added to water. Na 3 PO 4 + H 2 O! Na + + OH + HPO 4 2 ( or H 2 PO 4 ) 18. Solid lithium oxide is added to excess water. Li 2 O + H 2 O! Li + + OH 19. Solid barium oxide is added to distilled water. BaO + H 2 O! Ba 2+ + OH 20. Solid calcium hydride is added to distilled water. CaH 2 + H 2 O! Ca 2+ + OH or (Ca(OH) 2 ) + H 2 Combustion 1. Lithium metal is burned in air. Li + O 2! Li 2 O 2. The hydrocarbon hexane is burned in excess oxygen. C 6 H 14 + O 2! CO 2 + H 2 O 3. Gaseous diborane, B 2 H 6, is burned in excess oxygen. B 2 H 6 + O 2! B2 O 3 + H 2 O 4. A piece of solid bismuth is heated strongly in oxygen. Bi + O 2! Bi 2 O 3 5. Solid zinc sulfide is heated in an excess of oxygen. ZnS + O 2! ZnO + SO 2 6. Propanol is burned completely in air. C 3 H 7 OH + O 2! CO 2 + H 2 O 7. Excess oxygen gas is mixed with ammonia gas in the presence of platinum. O2 + NH 3 Pt! NO 2 + H 2 O 8. Gaseous silane, SiH 4, is burned in oxygen. Kristen Henry Jones 4
11 SiH 4 + O 2! SiO 2 + H 2 O 9. Ethanol is completely burned in air. C 2 H 5 OH + O 2! CO 2 + H 2 O 10. Solid copper(ii) sulfide is heated strongly in oxygen gas. CuS + O 2! CuO + SO Ethanol is burned in oxygen. C 2 H 5 OH + O 2! CO 2 + H 2 O Redox 1. Iron(III) ions are reduced by iodide ions. Fe 3+ + I! Fe 2+ + I 2 2. Potassium permanganate solution is added to concentrated hydrochloric acid. MnO 4 + H + + Cl! Mn 2+ + Cl 2 + H 2 O 3. Magnesium metal is added to dilute nitric acid, giving as one of the products a compound in which the oxidation number for nitrogen is 3. Mg + H + + NO 3! NH Mg 2+ + H 2 O 4. A solution of potassium iodide is electrolyzed. I + H 2 O! I 2 + H 2 + OH 5. Potassium dichromate solution is added to an acidified solution of sodium sulfite. Cr 2 O SO H +! Cr 3+ + SO H 2 O 6. Solutions of potassium iodide, potassium iodate, and dilute sulfuric acid are mixed. I + IO 3 + H +! H 2 O + I 2 7. A solution of tin(ii) sulfate is added to a solution of iron(iii) sulfate. Sn 2+ + Fe 3+!Sn 4+ + Fe Metallic copper is heated with concentrated sulfuric acid. Cu + H 2 SO 4! Cu 2+ + SO 2 + H 2 O 9. Manganese(IV) oxide is added to warm, concentrated hydrobromic acid. MnO 2 + H + + Br! Mn 2+ + Br 2 + H 2 O 10. Chlorine gas is bubbled into cold dilute sodium hydroxide. Cl 2 + OH! ClO + Cl + H 2 O 11. Solid iron(iii) oxide is heated in excess carbon monoxide. Fe 2 O 3 + CO!Fe + CO Hydrogen peroxide solution is added to acidified potassium iodide solution. H 2 O 2 + H + + I! H 2 O + I Hydrogen peroxide is added to an acidified solution of potassium dichromate. H 2 O 2 + H + + Cr 2 O 7 2! H2 O + Cr 3+ + O Sulfur dioxide gas is bubbled through an acidified solution of potassium permanganate. SO 2 + H + + MnO 4! Mn 2+ + H 2 O + SO A solution containing tin(ii) ions is added to an acidified solution of potassium dichromate. Sn 2+ + H + + Cr 2 O 7 2! Cr 3+ + Sn 4+ + H 2 O 16. Solid silver sulfide is warmed with dilute nitric acid. Ag 2 S + H + + NO 3! Ag + + S + NO 2 + H 2 O 17. A dilute solution of sulfuric acid is electrolyzed between platinum electrodes. H 2 O!H 2 + O Pellets of lead are dropped into hot sulfuric acid. Pb + H + + SO 4 2! H 2 O + SO 2 + Pb 2+ (or PbSO 4 ) Kristen Henry Jones 5
12 19. Potassium permanganate solution is added to a solution of oxalic acid, H 2 C 2 O 4, acidified with a few drops of sulfuric acid. MnO 4 + H 2 C 2 O 4 + H +! Mn 2+ + CO 2 + H 2 O 20. Powdered iron is added to a solution of iron(iii) sulfate. Fe + Fe 3+! Fe A concentrated solution of hydrochloric acid is added to powdered manganese dioxide and gently heated. H + + Cl + MnO 2! Cl 2 + Mn 2+ + H 2 O 22. A strip of copper metal is added to a concentrated solution of sulfuric acid. Cu + H + + SO 4 2! Cu 2+ + SO 2 + H 2 O 23. Copper(II) sulfide is oxidized by dilute nitric acid. CuS + H + + NO 3!Cu 2+ + NO + H 2 O + S 24. A solution of copper(ii) sulfate is electrolyzed using inert electrodes. Cu 2+ + H 2 O! O 2 + H + + Cu 25. A solution of potassium iodide is added to an acidified solution of potassium dichromate. I + H + + Cr 2 O 7 2! I 2 + Cr 3+ + H 2 O 26. Hydrogen peroxide solution is added to a solution of iron(ii) sulfate. H 2 O 2 + Fe 2+! Fe 3+ + H 2 O 27. Solid silver is added to a dilute nitric acid (6M) solution. Ag + H + +NO 3! Ag + + NO + H 2 O 28. A solution of formic acid, HCOOH, is oxidized by an acidified solution of potassium dichromate. HCOOH + H + + Cr 2 O 7 2! H 2 O + Cr 3+ + CO A piece of iron is added to a solution of iron(iii) sulfate. Fe + Fe 3+! Fe An acidified solution of potassium permanganate is added to a solution of sodium sulfite. H + + MnO 4 + SO 3 2! Mn 2+ + SO H 2 O 31. A solution of tin(ii) chloride is added to a solution of iron(iii) sulfate. Sn 2+ + Fe 3+! Sn 4+ + Fe Concentrated hydrochloric acid solution is added to solid manganese(iv) oxide and the reactants are heated. H + + Cl + MnO 2! Mn 2+ + Cl 2 + H 2 O 33. A strip of copper is immersed in dilute nitric acid. Cu + H + + NO 3! Cu 2+ + NO + H 2 O 34. Potassium permanganate solution is added to an acidic solution of hydrogen peroxide. MnO 4 + H + + H 2 O 2! Mn 2+ + O 2 + H 2 O 35. Solid copper is added to a dilute nitric acid solution. Cu + H + + NO 3! Cu 2+ + NO + H 2 O 36. Chlorine gas is bubbled into a cold solution of dilute sodium hydroxide. Cl 2 + OH!ClO + Cl + H 2 O 37. A solution of potassium permanganate is mixed with an alkaline solution of sodium sulfite. MnO 4 + OH + SO 3 2! SO H 2 O + MnO 4 2 (or MnO 2 ) 38. Solid sodium dichromate is added to an acidified solution of sodium iodide. Na 2 Cr 2 O 7 + H + + I! Cr 3+ + I 2 + H 2 O + Na Hydrogen gas is passed over hot iron(iii) oxide. Kristen Henry Jones 6
13 H 2 + Fe 2 O 3! Fe + H 2 O 40. Solutions of potassium iodide and potassium iodate are mixed in acid solution. I + IO 3 + H +! I 2 + H 2 O 41. Hydrogen peroxide is added to an acidified solution of sodium bromide. H 2 O 2 + H + + Br! Br 2 + H 2 O 42. Chlorine gas is bubbled into a cold, dilute solution of potassium hydroxide. Cl 2 + OH! Cl + ClO + H 2 O 43. A solution of iron(ii) nitrate is exposed to air for an extended period of time. Fe 2+ + O 2! Fe 2 O 3 AcidBase Neutralizations 1. Solutions of ammonia and hydrofluoric acid are mixed. NH 3 + HF! NH F 2. Hydrogen sulfide gas is bubbled through a solution of potassium hydroxide. H 2 S + OH! H 2 O + S 2 3. A solution of sulfuric acid is added to a solution of barium hydroxide until the same number of moles of each compound has been added. H + + SO Ba 2+ + OH! H 2 O + BaSO 4 4. A solution of sodium hydroxide is added to a solution of sodium dihydrogen phosphate until the same number of moles of each compound has been added. OH + H 2 PO 4! HPO H 2 O 5. Dilute nitric acid is added to crystals of pure calcium oxide. H + + CaO! H 2 O + Ca Equal volumes of 0.1molar sulfuric acid and 0.1molar potassium hydroxide are mixed. H + +OH! H 2 O 7. A solution of ammonia is added to a dilute solution of acetic acid. NH 3 + HC 2 H 3 O 2! NH C 2 H 3 O 2 8. Excess sulfur dioxide gas is bubbled through a dilute solution of potassium hydroxide. SO 2 + OH! H 2 O + SO Sulfur dioxide gas is bubbled into an excess of a saturated solution of calcium hydroxide. SO 2 + Ca 2+ + OH! CaSO 3 + H 2 O 10. A solution of sodium hydroxide is added to a solution of calcium hydrogen carbonate until the number of moles of sodium hydroxide added is twice the number of moles of the calcium salt. OH +Ca 2+ + HCO 3! H 2 O + CaCO Equal volumes of 0.1M hydrochloric acid and 0.1M sodium monohydrogen phosphate are mixed. H + + HPO 4 2! H 2 PO Hydrogen sulfide gas is bubbled through excess potassium hydroxide solution. H 2 S + OH! H 2 O + S Ammonia gas and carbon dioxide gas are bubbled into water. NH 3 + CO 2 + H 2 O! NH CO Carbon dioxide gas is bubbled through a concentrated solution of sodium hydroxide. CO 2 + OH! CO H 2 O 15. Acetic acid solution is added to a solution of sodium hydrogen carbonate. HC 2 H 3 O 2 + HCO 3! H 2 O + CO 2 + C 2 H 3 O 2 Kristen Henry Jones 7
14 16. Excess potassium hydroxide solution is added to a solution of potassium dihydrogen phosphate. OH + H 2 PO 4! H 2 O + PO 4 3 Complex Ions 1. Concentrated (15M) ammonia solution is added in excess to a solution of copper(ii) nitrate. NH 3 + Cu 2+! [Cu(NH 3 ) 4 ] An excess of nitric acid solution is added to a solution of tetraaminecopper(ii) sulfate. H + + [Cu(NH 3 ) 4 ] 2+! NH Cu Dilute hydrochloric acid is added to a solution of diamminesilver(i) nitrate. H + + Cl + [Ag(NH 3 ) 2 ] +! AgCl + NH Solid aluminum nitrate is dissolved in water. Al(NO 3 ) 3 + H 2 O! [Al(H 2 O) 6 ] +3 + NO 3 5. A suspension of copper(ii) hydroxide is treated with an excess of ammonia water. Cu(OH) 2 + NH 3! [Cu(NH 3 ) 4 ] 2+ + OH 6. A solution of diamminesilver(i) chloride is treated with dilute nitric acid. [Ag(NH 3 ) 2 ] + + Cl + H +! NH AgCl 7. An excess of concentrated ammonia solution is added to freshly precipitated copper(ii) hydroxide. NH 3 + Cu(OH) 2! [Cu(NH 3 ) 4 ] 2+ + OH 8. Excess dilute nitric acid is added to a solution containing the tetraaminecadmium(ii) ion. H + + [Cd(NH 3 ) 4 ] 2+! NH Cd An excess of ammonia is bubbled through a solution saturated with silver chloride. NH 3 + Ag +! [Ag(NH 3 ) 2 ] Solid aluminum oxide is added to a solution of sodium hydroxide. Al 2 O 3 + OH! [Al(OH) 4 ] (may have water as a reactant) 11. A concentrated solution of ammonia is added to a solution of zinc iodide. NH 3 + Zn 2+! [Zn(NH 3 ) 4 ] An excess of sodium hydroxide solution is added to a solution of aluminum chloride. OH + Al 3+! [Al(OH) 4 ] 13. A concentrated solution of ammonia is added to a solution of copper(ii) chloride. NH 3 + Cu 2+! [Cu(NH 3 ) 4 ] Excess concentrated sodium hydroxide solution is added to solid aluminum hydroxide. OH + Al(OH) 3! [Al(OH) 4 ] 15. Excess concentrated ammonia solution is added to a suspension of silver chloride. NH 3 + AgCl! [Ag(NH 3 ) 2 ] + + Cl 16. Pellets of aluminum metal are added to a solution containing an excess of sodium hydroxide. Al + OH! [Al(OH) 4 ] 17. A suspension of zinc hydroxide is treated with concentrated sodium hydroxide solution. Zn(OH) 2 + OH! [Zn(OH) 4 ] Silver chloride is dissolved in excess ammonia solution. AgCl + NH 3! [Ag(NH 3 ) 2 ] + + Cl 19. Sodium hydroxide solution is added to a precipitate of aluminum hydroxide in water. OH + Al(OH) 3! [Al(OH) 4 ] 20. A drop of potassium thiocyanate is added to a solution of iron(iii) chloride. Kristen Henry Jones 8
15 SCN + Fe 3+! FeSCN A concentrated solution of ammonia is added to a suspension of zinc hydroxide. NH 3 + Zn(OH) 2! [Zn(NH 3 ) 4 ] 2+ + OH 22. Excess concentrated potassium hydroxide solution is added to a precipitate of zinc hydroxide. Zn(OH) 2 + OH! [Zn(OH) 4 ] 2 Addition 1. The gases boron trifluoride and ammonia are mixed. BF 3 + NH 3! F 3 BNH 3 2. A mixture of solid calcium oxide and solid tetraphosphorus decaoxide is heated. CaO + P 4 O 10! Ca 3 (PO 4 ) 2 3. Solid calcium oxide is exposed to a stream of carbon dioxide gas. CaO + CO 2! CaCO 3 4. Solid calcium oxide is heated in the presence of sulfur trioxide gas. CaO + SO 3! CaSO 4 5. Calcium metal is heated strongly in nitrogen gas. Ca + N 2! Ca 3 N 2 6. Excess chlorine gas is passed over hot iron filings. Cl 2 + Fe! FeCl 3 7. Powdered magnesium oxide is added to a container of carbon dioxide gas. MgO + CO 2! MgCO 3 8. A piece of lithium metal is dropped into a container of nitrogen gas. Li + N 2! Li 3 N 9. Magnesium metal is burned in nitrogen gas. Mg + N 2! Mg 3 N Sulfur dioxide gas is passed over solid calcium oxide. SO 2 + CaO! CaSO 3 Decomposition 1. A solution of hydrogen peroxide is heated. H 2 O 2! O 2 + H 2 O 2. Solid magnesium carbonate is heated. MgCO 3! MgO + CO 2 3. A solution of hydrogen peroxide is catalytically decomposed. H 2 O 2! H 2 O + O 2 Kristen Henry Jones 9
16 4. Solid potassium chlorate is heated in the presence of manganese dioxide as a catalyst. KClO 3! MnO! 2 " KCl + O 2 5. Sodium hydrogen carbonate is dissolved in water. NaHCO 3! Na + + HCO 3 6. Solid ammonium carbonate is heated. (NH 4 ) 2 CO 3! CO 2 + NH 3 + H 2 O ORGANIC 1. A sample of pure 2butene is treated with hydrogen bromide gas. C 4 H 8 + HBr! C 4 H 9 Br 2. An excess of chlorine gas is added to pure acetylene. Cl 2 + C 2 H 2! C 2 H 2 Cl 4 3. Ethyl acetate is treated with a solution of sodium hydroxide. CH 3 COOC 2 H 5 + OH! C 2 H 5 OH + CH 3 COO 4. Benzene is treated with bromine in the presence of a catalyst. Br 2 + C 6 H 6! C 6 H 5 Br + HBr 5. Propene reacts with water in the presence of a catalyst. C 3 H 6 + H 2 O! C 3 H 7 OH 6. Methyl iodide is heated with a solution of sodium hydroxide. CH 3 I + OH! CH 3 OH + I 7. Methane gas is heated with an excess of chlorine gas. CH 4 + Cl 2! CH 3 Cl + HCl 8. Ethanol and formic acid (methanoic acid) are mixed and warmed. C 2 H 5 OH + HCOOH! HCOOC 2 H 5 + H 2 O 9. Ethene (ethylene) gas is bubbled through a solution of bromine. C 2 H 4 + Br 2! C 2 H 4 Br 2 Kristen Henry Jones 10
Decomposition. Composition
Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus
More informationAP Chemistry Reaction Questions
AP Chemistry Reaction Questions Directions: Give the formulas to show the reactants and the products for the following chemical reactions. Each of the reactions occurs in aqueous solution unless otherwise
More informationWRITING AP EQUATIONS
WRITING AP EQUATIONS AP equation sets are found in the free-response section of the AP test. This is a 15 point question and you can practice for it all year! You are given three equations and you must
More informationBalancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
More informationHOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions
HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
More informationNaming Compounds Handout Key
Naming Compounds Handout Key p. 2 Name each of the following monatomic cations: Li + = lithium ion Ag + = silver ion Cd +2 = cadmium ion Cu +2 = copper (II) ion Al +3 = aluminum ion Mg +2 = magnesium ion
More informationSCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
More informationNomenclature of Ionic Compounds
Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons.
More informationDavid A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationNAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide
NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate
More informationTutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE
T-6 Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE FORMULAS: A chemical formula shows the elemental composition of a substance: the chemical symbols show what elements are present and the numerical
More informationMoles, Molecules, and Grams Worksheet Answer Key
Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3
More informationChapter 16: Tests for ions and gases
The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the
More informationNaming Ionic Compounds
Naming Ionic Compounds I. Naming Ions A. Cations (+ions) 1. Element name followed by "ion" (when in Group IA, IIA, Al 3+, Ga 3+, Zn 2+, Cd 2+, Ag +, Ni 2+ ). Na + sodium ion, K + potassium ion, Al 3+ aluminum
More informationCHEMICAL NAMES AND FORMULAS
9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages 253 258) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the
More informationUnit 9 Stoichiometry Notes (The Mole Continues)
Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationExperiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
More informationMonatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on
More informationNomenclature Packet. 1. Name the following ionic compounds: a. Al 2 O 3 Aluminum oxide. b. Cs 2 O Cesium oxide. c. Rb 3 N Rubidium nitride
Nomenclature Packet Worksheet I: Binary Ionic Compounds (representative metals) metals from groups 1A, 2A, and 3A (1, 2, and 13) have constant charges as ions and do NOT get Roman Numerals in their names
More informationNaming Compounds. There are three steps involved in naming ionic compounds- naming the cation, naming the anion, and naming the entire compound.
Naming Compounds Naming compounds is an important part of chemistry. Most compounds fall in to one of three categories ionic compounds, molecular compounds, or acids. Part One: Naming Ionic Compounds Identifying
More informationChemistry Themed. Types of Reactions
Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start
More informationStoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More informationCHAPTER 5: MOLECULES AND COMPOUNDS
CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting
More informationElectrochemistry - ANSWERS
Electrochemistry - ANSWERS 1. Using a table of standard electrode potentials, predict if the following reactions will occur spontaneously as written. a) Al 3+ + Ni Ni 2+ + Al Al 3+ + 3e - Al E = -1.68
More informationChapter 6 Notes Science 10 Name:
6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and
More informationNomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula
Purpose: Theory: Nomenclature and Formulas of Ionic Compounds 1. To become familiar with the rules of chemical nomenclature, based on the classification of compounds. 2. To write the proper name of the
More informationWRITING CHEMICAL FORMULA
WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.
More informationExperiment 1 Chemical Reactions and Net Ionic Equations
Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical
More informationChapter 8 - Chemical Equations and Reactions
Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from
More informationWriting and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
More informationMoles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
More informationName: Block: Date: Test Review: Chapter 8 Ionic Bonding
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Part 1: Fill-in-the-blank. Choose the word from the word bank below. Each word may be used only 1 time. electron dot structure metallic electronegativity
More informationCHEM 1411 General Chemistry I Practice Problems, Chapters 1 3
CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3 Chapter 1 Chemistry: The Study of Change 1. Element, compound, homogeneous mixture (solution), or heterogeneous mixture: a) orange juice b)
More informationSanta Monica College Chemistry 11
Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical
More information= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
More informationW1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
More informationSolution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent
Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:
More informationOxidation States of Nitrogen
Oxidation States of Nitrogen HNO 3 NH 3 HNO 2 NO N 2 O N 2 HN 3 N 2 H 5 + +3 +2 +1 0-1/3-2 Oxidation +5-3 Reduction Oxidation States of Chlorine HClO 4 HClO 3 ClO 2 HClO 2 HClO Cl 2 HCl +5 +4 +3 +1 0 Oxidation
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More informationChapter 4 Compounds and Their Bonds
Chapter 4 Compounds and Their Bonds 4.1 Octet Rule and Ions Octet Rule An octet is 8 valence electrons. is associated with the stability of the noble gases. He is stable with 2 valence electrons (duet).
More informationneutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
More informationTopic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole
Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present
More informationProblem Solving. Stoichiometry of Gases
Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.
More informationMolar Mass Worksheet Answer Key
Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl 3 162.3 g/mol 5) BF 3 67.8 g/mol 6) CCl 2 F 2 121 g/mol
More informationName period Unit 3 worksheet
Name period Unit 3 worksheet Read chapter 8, 2.52.7 1. Explain the difference between metallic, ionic, and covalent bonding Metallic cations share a sea of electrons Ionic atoms give and take electrons
More information1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
More informationNaming Ionic Compounds Answer Key
Naming Ionic Compounds Answer Key Give the name of the following ionic compounds: Name 1) Na 2 CO 3 sodium carbonate 2) NaOH sodium hydroxide 3) MgBr 2 magnesium bromide 4) KCl potassium chloride 5) FeCl
More informationChapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
More informationNumber of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V
44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts
More informationChemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
More informationPART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)
CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students
More informationGeneral Chemistry Lab Experiment 6 Types of Chemical Reaction
General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more
More informationProblem Solving. Percentage Composition
Skills Worksheet Problem Solving Percentage Composition Suppose you are working in an industrial laboratory. Your supervisor gives you a bottle containing a white crystalline compound and asks you to determine
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationExercise 3.5 - Naming Binary Covalent Compounds:
Chapter Exercise Key 1 Chapter Exercise Key Exercise.1 Classifying Compounds: Classify each of the following substances as either a molecular compound or an ionic compound. a. formaldehyde, CH 2 O (used
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationChapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
More informationSample Exercise 2.1 Illustrating the Size of an Atom
Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side
More informationChapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction
Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,
More informationChapter 7: Chemical Reactions
Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that
More information1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11
SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436
More informationDepartment of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources
Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources Introduction This document is intended to help you review the basics of writing
More informationMolarity of Ions in Solution
APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.
More informationChapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
More informationMOLES AND MOLE CALCULATIONS
35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product
More informationFORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p. 56-63 and the 1411 Lab Manual, p. 27-31.
FORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p. 56-63 and the 1411 Lab Manual, p. 27-31. TYPES OF COMPOUNDS Ionic compounds are compounds composed of
More informationCHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals
CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
More informationAqueous Ions and Reactions
Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for
More informationAPPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
More informationCHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
More informationProblem Solving. Mole Concept
Skills Worksheet Problem Solving Mole Concept Suppose you want to carry out a reaction that requires combining one atom of iron with one atom of sulfur. How much iron should you use? How much sulfur? When
More informationUNIT (4) CALCULATIONS AND CHEMICAL REACTIONS
UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12
More informationPeriodic Table, Valency and Formula
Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed
More informationSEATTLE CENTRAL COMMUNITY COLLEGE DIVISION OF SCIENCE AND MATHEMATICS. Oxidation-Reduction
SEATTLE CENTRAL COMMUNITY COLLEGE DIVISION OF SCIENCE AND MATHEMATICS OxidationReduction Oxidation is loss of electrons. (Oxygen is EN enough to grab e away from most elements, so the term originally meant
More informationEDULABZ. Na 2 + H 2 CO 3. O + CO 2 (b) CaO + H 2. + NaCl AgCl + NaNO 3 3. Which of the following reactions does not take place?
4 TRANSFORMATION OF SUBSTANCE I. Multiple choice questions: (Tick the correct option). 1. The reaction between magnesium and oxygen is: (a) an endothermic reaction (b) an exothermic reaction (c) a catalysed
More information80. Testing salts for anions and cations
Classic chemistry experiments 203 80. Testing salts for anions and cations Topic Qualitative analysis. Timing Description 12 hours. Students attempt to identify the anions and cations present in a salt
More informationChemical Reactions. Section 9.1 Reactions and Equations pages 282 288 SOLUTIONS MANUAL. Practice Problems pages 284 287
CHAPTER 9 Chemical Reactions Section 9.1 Reactions and Equations pages 282 288 Practice Problems pages 284 287 Write skeleton equations for the following word equations. 1. Hydrogen and bromine gases react
More informationFormulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
More informationGCE. Moles, Formulae and Equations Edexcel Advanced GCE in Chemistry (9080) Edexcel Advanced GCE in Chemistry (Nuffield) (9086) Issue 3 October 2004
GCE Moles, Formulae and Equations Edexcel Advanced GCE in Chemistry (Nuffield) (9086) Issue 3 October 2004 Workbook for GCE students GCE Moles, Formulae and Equations Edexcel Advanced GCE in Chemistry
More informationChapter 3 Chemical Compounds
Chapter 3 Chemical Compounds 3.1 (a) formula unit; (b) strong electrolyte; (c) molecular compound; (d) acid; (e) nonelectrolyte; (f) oxoanion 3.2 (a) molecular formula; (b) weak electrolyte; (c) ionic
More informationCHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES
CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES The meaning of stoichiometric coefficients: 2 H 2 (g) + O 2 (g) 2 H 2 O(l) number of reacting particles 2 molecules of hydrogen react with 1 molecule
More informationExperiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
More informationChapter 6: Writing and Balancing Chemical Equations. AB A + B. CaCO3 CaO + CO2 A + B C. AB + C AC + B (or AB + C CB + A)
78 Chapter 6: Writing and Balancing Chemical Equations. It is convenient to classify chemical reactions into one of several general types. Some of the more common, important, reactions are shown below.
More information4. Balanced chemical equations tell us in what molar ratios substances combine to form products, not in what mass proportions they combine.
CHAPTER 9 1. The coefficients of the balanced chemical equation for a reaction give the relative numbers of molecules of reactants and products that are involved in the reaction.. The coefficients of the
More informationChapter 12: Oxidation and Reduction.
207 Oxidation- reduction (redox) reactions Chapter 12: Oxidation and Reduction. At different times, oxidation and reduction (redox) have had different, but complimentary, definitions. Compare the following
More informationModule Four Balancing Chemical Reactions. Chem 170. Stoichiometric Calculations. Module Four. Balancing Chemical Reactions
Chem 170 Stoichiometric Calculations Module Four Balancing Chemical Reactions DePauw University Department of Chemistry and Biochemistry Page 1 Introduction to Module Four When making a cheeseburger you
More informationb. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.
CHEMISTRY DISCOVER UNIT 5 LOTS OF PRACTICE ON USING THE MOLE!!! PART 1: ATOMIC MASS, FORMULA MASS, OR MOLECULAR MASS 1. Determine the atomic mass, formula mass, or molecular mass for each of the following
More informationPolyatomic ions can form ionic compounds just as monatomic ions.
1 POLYATOMIC IONS We have seen that atoms can lose or gain electrons to become ions. Groups of atoms can also become ions. These groups of atoms are called polyatomic ions. Examples: O hydroxide ion NO
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More information1332 CHAPTER 18 Sample Questions
1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+
More informationChapter 1: Moles and equations. Learning outcomes. you should be able to:
Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including
More informationElements and Compounds. Chemical Bonds compounds are made of atoms held together by chemical bonds bonds are forces of attraction between atoms
Elements and Compounds elements combine together to make an almost limitless number of compounds the properties of the compound are totally different from the constituent elements Tro, Chemistry: A Molecular
More informationAtomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells
Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This
More informationName period Unit 9: acid/base equilibrium
Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton
More informationConcept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.
Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of
More information